Answer:
Water
Explanation:
This is because it only contains one type of molecule.
Answer:
12.6.
Explanation:
- We should calculate the no. of millimoles of KOH and HCl:
no. of millimoles of KOH = (MV)KOH = (0.183 M)(45.0 mL) = 8.235 mmol.
no. of millimoles of HCl = (MV)HCl = (0.145 M)(35.0 mL) = 5.075 mmol.
- It is clear that the no. of millimoles of KOH is higher than that of HCl:
So,
[OH⁻] = [(no. of millimoles of KOH) - (no. of millimoles of HCl)] / (V total) = (8.235 mmol - 5.075 mmol) / (80.0 mL) = 0.395 M.
∵ pOH = -log[OH⁻]
∴ pOH = -log(0.395 M) = 1.4.
∵ pH + pOH = 14.
∴ pH = 14 - pOH = 14 - 1.4 = 12.6.
Answer:
P(H₂) = 0.8533 atm
Explanation:
n(CO) = 0.220 mole
n(H₂) = 0.350 mole
n(He) = 0.640 mole
_______________
∑ n = 1.210 moles
mole fraction => X(H₂) = 0.350/1.210 = 0.2892
Dalton's Law of Partial Pressures => P(H₂) = X(H₂)·P(ttl) = 0.2892(2.95 atm) = 0.8533 atm
Answer:
38 moles of oxygen
Explanation:
<em>This is the chemical formula for nickel tetracarbonyl (a powerfully poisonous liquid used in nickel refining): Ni(CO)₄. A chemical engineer has determined by measurements that there are 9.6 moles of nickel in a sample of nickel tetracarbonyl. How many moles of oxygen are in the sample?</em>
Step 1: Given data
Chemical formula of nickel tetracarbonyl: Ni(CO)₄
Moles of nickel: 9.6 moles
Step 2: Establish the molar ratio of nickel to oxygen
According to the chemical formula, the molar ratio of nickel to oxygen is 1:4.
Step 3: Calculate the moles of oxygen that accompany 9.6 moles of nickel.
We will use the previously established molar ratio.
9.6 mol Ni × (4 mol O/1 mol Ni) = 38 mol O