S, sulfur does not have a noble gas electron.
Answer:
The answer is: 51.8 g (86% of serving size)
Explanation:
In order to solve the problem, we have to first determine the number of moles there are in 11.0 g of sucrose. Sucrose has a molecular weight of 342 g (we calculate this from the molar mass of the elements : 12 x 12 g/mol C + 22 x 1 g/mol H + 11 x 16 g/mol O). So, we divide the mass (11.0 g) into the molecular weight of sucrose:
11.0 g sucrose x 1 mol/342 g sucrose= 0.032 mol
We have 0.032 mol of sucrose in a serving of 60 g. But we need less moles (0.0278 mol):
0.032 mol ------------ 60 g serving
0.0278 mol------------ x= 0.0278 mol x 60 g serving/0.032 mol
x= 51.8 g
So, lesser than 1 serving of 60 g must be eaten to consume 0.0278 mol os sucrose. Exactly, 51.8 g (which stands for a 86% of the serving size).
Answer:
2.88moles
Explanation:
To solve this question adequately, we need to have a balanced chemical equation
2Cu2O + Cu2S → 6Cu + SO2
From the chemical equation, we can see that the mole ratio of the sulfur oxide to the Cu is 6 to 1.
This means that if 0.48 mole is sulfur oxide is produced, then 6 of this number of moles would have been produced in the case of Cu.
Hence, to get the number of moles of copper produced, we simply multiply 0.48 by 6 to give 2.88 moles
