These are two questions and two answers.
Answers:
Explanation:
<u>1) Balanced chemical equation (given):</u>
- CO₂(g) + 4H₂(g) → CH₄(g) + 2H₂O(g)
<u>2) Part A: How many moles of methane are produced when 59.6 moles of carbon dioxide gas react with excess hydrogen gas? </u>
a)<u> Mole ratios:</u>
- 1 moles CO₂(g) : 1 mole CH₄(g)
b) <u>Proportion:</u>
- 1 moles CO₂ / 1 mol CH₄ = 59.6 moles CO₂ / x
⇒ x = 59.6 mol CH₄ ← answer
<u>3) Part B How many moles of hydrogen gas would be needed to react with excess carbon dioxide to produce 42.1 moles of water vapor? </u>
a) <u>Mole ratios:</u>
- 4 mol H₂(g) : 2 mol H₂O(g)
b) <u>Proportion:</u>
- 4 mol H₂ / 2 mol H₂O = x / 42.1 mol H₂O
⇒ x = 42.1 × 4 / 2 moles CH₄ = 84.2 mol H₂ (g) ← answer
You don’t have any charge outside of the nuclear
15.0 meters = 15,000 millimeters
Answer:
8.75 mL
Explanation:
First, we calculate the molar mass of NaCl = molar mass of Na + molar mass of Cl. Molar mass of Na = 23 g/mol, molar mass of Cl = 35.5 g/mol.
So molar mass NaCl = (23 + 35.5) g/mol = 58.5 g/mol. The number of moles ,n of NaCl in 12.5g is n = mass of NaCl/ molar mass NaCl = 12.5 g / 58.5 g/mol = 0.214 mol.
The molarity, M of 150 mL M = number of moles/ volume = 0.214 mol / 150 mL = 1.427 M.
We now calculate the number of moles of NaCl in 250 mL of 0.500 M.
Number of moles, n = molarity × volume. molarity = 0.500 M, volume = 250 mL. So n = 0.500 × 250 = 0.125 moles. Since we have 0.125 moles in the dilute 250 mL solution, the volume of the 150 mL 1.43 M solution required is number of moles in 250 mL solution/molarity of 150 mL solution = 0.125 mol / 1.427 M = 0.0875 L = 8.75 mL
You would use a mass spectrometer