A. 8.0g
B. 16.0g
C. 36.0g
D. 72.0g
QUICK ANSWER…
D
DETAILS…
To resolve this, we must write out the balanced equation thus: 2H₂ + O₂→ 2H₂O
From this balanced equation we can infer that:
2 moles of hydrogen is required to form 2 moles of water
Now, we have to determine how many moles of hydrogen is equivalent to a mass of 8g
2g of H₂ = 1 mole, therefore,
8g of H₂ = x mole.
Cross multiplying to solve for x, we have:
2x = 8
x = 8/2 = 4moles
this implies that 4 moles of hydrogen is present.
Now, if from the balanced equation,
2 moles of H₂ forms 2 moles of H₂O, then
4 moles of H₂ will form Y moles of H₂O
Cross multiplying to find Y, we have:
2Y = 4(2) = 8
Y = 8/2 = 4
This implies that the number of moles of water formed = 4 moles.
Now converting these 4 moles of water to grams, we have:
Molar mass of H₂O = 2 + 16 = 18g
This implies that 1 mole of H₂O = 18g, therefore,
4 moles will be = 4 × 18 = 72g
SHORT-CUT
There’s a short cut solution,
using the balanced equation,
2H₂ + O₂→ 2H₂O
mass of 2H₂ = 2(2) = 4g
mass of 2H₂O = 2(2+16) = 2(18) = 36g
this implies that:
4g of hydrogen gas produces 36g of water, therefore,
8g of hydrogen gas will produce X
cross multiplying to solve for X, we have:
X(4) = 8(36)
X = (8 × 36)/4 = 72g
Now for the right answer to the above question:
- Option A is incorrect.
- Option B is incorrect.
- C is incorrect.
- D is the correct answer.
KEY-POINTS…
You may please note these/this:
- For accuracy and clarity purposes, you must write out the balanced chemical equation of questions like this.
- The importance of writing out the balanced equation is to properly understand the mole ratios involved, and to make your assumptions properly.
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/ culled from 2020 JAMB-UTME chemistry past question 32 /
Therefore, 8 g of H2 is 4 moles. Therefore you will form 4 moles of water. The molar mass of water is 18 g/mol so you will form 4 x 18 = 72 g of water.
What is the total mass of water formed when 8 grams of hydrogen react with 64 grams of oxygen?, 1 g H2 reacts with= 8 g Oxygen. So 64 g of oxygen reacts with= 8 g H2. So (64+8)=72 g of water will be formed.
Furthermore, What is the total mass of water formed when 8 grams of hydrogen reacts completely with?, Answer: The total mass in grams of water formed when 8.00 grams of hydrogen reacts completely with excess oxygen is 71.5 g.
Finally, What weight of water is formed when 8 grams hydrogen and 8 g oxygen react together?, The molar mass of hydrogen is 2, oxygen is 32 and water is 18. Hence, with 8 grams of both hydrogen and oxygen, the mass of water produced is 9 gram.
Frequently Asked Question:
The explanation is: The chemical equation of water formation is 2H2 + O2 → 2H2O. Though we have 8g of hydrogen, here oxygen is the limiting reagent. So the only 4g of hydrogen can be used to produce water i.e. 36g of water. That is 2 moles.
2 Answers. ≈70 g H2O will produced from 8 g H2 .
The molecular masses of hydrogen, oxygen and water are 2 g/mole, 32 g/mole and 18 g/mole respectively. 2×2=4 g of hydrogen reacts with 1×32=32 g of oxygen to form 2×18=36 g of water. =9 g of water. 9 grams of water can be produced when 8 g of hydrogen reacts with 8 g oxygen.
2 Answers. ≈70 g H2O will produced from 8 g H2 .
The molecular masses of hydrogen, oxygen and water are 2 g/mole, 32 g/mole and 18 g/mole respectively. 2×2=4 g of hydrogen reacts with 1×32=32 g of oxygen to form 2×18=36 g of water. =9 g of water. 9 grams of water can be produced when 8 g of hydrogen reacts with 8 g oxygen.
1 g H2 reacts with= 8 g Oxygen. So 64 g of oxygen reacts with= 8 g H2. So (64+8)=72 g of water will be formed.
So 8 g of oxygen will react with 1 g of hydrogen to produce 9 g of water.
The molecular masses of hydrogen, oxygen and water are 2 g/mole, 32 g/mole and 18 g/mole respectively. 2×2=4 g of hydrogen reacts with 1×32=32 g of oxygen to form 2×18=36 g of water. =9 g of water. 9 grams of water can be produced when 8 g of hydrogen reacts with 8 g oxygen.
2 Answers. ≈70 g H2O will produced from 8 g H2 .
So 32g of Oxygen reacts with 4 g of Hydrogen. Therefore 16 g of oxygen reacts with 2 g of Hydrogen and will form 18 g of water.
Hence, with 8 grams of both hydrogen and oxygen, the mass of water produced is 9 gram.
The explanation is: The chemical equation of water formation is 2H2 + O2 → 2H2O. Though we have 8g of hydrogen, here oxygen is the limiting reagent. So the only 4g of hydrogen can be used to produce water i.e. 36g of water.
2 Answers. ≈70 g H2O will produced from 8 g H2 .
32g O2 x 36.03056g H20/31.9988g O2 this way the O2 cancels out and you are left with just the H2O so your raw answer would be 36.0319112, then if your instructor requires a significant figure answer that would be to 2 significant figures the information you were given 32g O2, so as above 36g or Water are produced.
Answer: The total mass in grams of water formed when 8.00 grams of hydrogen reacts completely with excess oxygen is 71.5 g.
The molecular masses of hydrogen, oxygen and water are 2 g/mole, 32 g/mole and 18 g/mole respectively. 2×2=4 g of hydrogen reacts with 1×32=32 g of oxygen to form 2×18=36 g of water. =9 g of water. 9 grams of water can be produced when 8 g of hydrogen reacts with 8 g oxygen.
2 Answers. ≈70 g H2O will produced from 8 g H2 .
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Let's start by writing the balanced reaction equation:
2H2 + O2 "\\rightarrow" 2H2O
As one can see, when there is enough oxygen, 2 molecules of hydrogen give 2 molecules of water. Therefore, when there is enough oxygen, the number of the moles of hydrogen reacted equals the number of the moles of water produced:
"n \\text{ (H}_2\\text{)} = n \\text{ (H}_2\\text{O)}"
Let's calculate the number of the moles of hydrogen in 8.00 grams of hydrogen (the number of the moles is mass "m" divided by molar mass "M", "M"(H2) =2.01568 g/mol):
"n \\text{ (H}_2\\text{)}= \\frac{m}{M} = \\frac{8.00}{2.01568} = 3.97" mol
"n \\text{ (H}_2\\text{O)} = 3.97" mol
The molar mass of water is 18.01528 g/mol. The mass of water produced is:
"m = n\\cdot M = 3.97 \\cdot 18.01528 = 71.5" g
Answer: The total mass in grams of water formed when 8.00 grams of hydrogen reacts completely with excess oxygen is 71.5 g.