Question

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.

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

Answer 2

Answer:

Moles of SnO2 = 0.020

Explanation:

Given:

SnO2 (s) + 2H2(g) → Sn(l) + 2H2O(g)

Mass of SnO2 = 3.00 g

Molar mass of SnO2 = 151 g/mol

Explanation:

'Mole' refers to the amount of a given substance. It is expressed in terms of the ratio of the mass of the substance to its molar mass

$Mole = \frac{Mass (g)}{Molar\ Mass (g/mol)} \\\\Moles\ SnO2 = \frac{3.00 g}{151 g/mol } = 0.0198\ moles = 0.020\ moles$