Base your answer to the question on the information below and on your knowledge of chemistry. At 1023 K and 1 atm, a 3.00-gram sample of SnO2 (s) (gram formula mass = 151 g/mol) reacts with hydrogen gas to produce tin and water, as shown in the balanced equation below. SnO2 (s) + 2H2 (g) → Sn (L) + 2H2O (g) Show a numerical setup for calculating the number of moles of SnO2 (s) in the 3.00-gram sample.

Question

Chemistry

Cooper Atkinson

10 June, 05:29

Base your answer to the question on the information below and on your knowledge of chemistry. At 1023 K and 1 atm, a 3.00-gram sample of SnO2 (s) (gram formula mass = 151 g/mol) reacts with hydrogen gas to produce tin and water, as shown in the balanced equation below. SnO2 (s) + 2H2 (g) → Sn (L) + 2H2O (g) Show a numerical setup for calculating the number of moles of SnO2 (s) in the 3.00-gram sample.

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Roberson · Answer 1

To calculate for the number of moles of SnO2 in the sample, we need the value of the products from the reaction. Since we do not have that data, we can assume that all of the sample is SnO2. Then, we are given the molecular mass of the sample, 151g/mol.

So, the number of moles is 3g / 151 g/mol = 0.0199 moles SnO2