Answer: 5.47x10^24 molecules
Explanation:
6.02214076x10^23 molecules CO2 = 44g
400g = (400/44)*6.02214076*10^23 = 5.47x10^24
The mass of that would be formed will be 18.22 grams
<h3>Stoichiometric calculations</h3>
Let us first look at the balanced equation of the reaction:
The mole ratio of Y to is 2:3.
Mole of 10.0 grams of Y = 10/88.9 = 0.11 moles
Mole of 10.0 grams = 10/71 = 0.14 moles
3/2 of 0.11 = 0.165. Thus, is limiting in availability.
Mole ratio of and = 3:2
Equivalent mole of = 2/3 x 0.14 = 0.093 moles.
Mass of 0.093 moles =0.093 x 195.26 = 18.22 grams
More on stoichiometric calculations can be found here: brainly.com/question/27287858
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Answer:
2Mg^+ +O2 right arrow 2MgO
Explanation:
Answer:
2.0 x 10^-2 L
Explanation:
PV=nRT
Substitute values into the ideal gas equation.
P = 780 kPa
V = ?
n = 21 mol
R = 8.314 L-kPa/mol-K
T = 900 K
(780 kPa)(V) = (21 mol)(8.314 L-kPa/mol-K)(900 K)
V = (21 mol)(8.314 L-kPa/mol-K)(900K) / (780 kPa)
V = 201.4561...
Round to sig figs.
V = 2.0 x 10^2 L
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