Answer:
Option D.
Explanation:
Let's apply the Ideal Gases law to solve the problem.
P . V = n . R . T
First of all we convert the temperature value from °C to K
77°C + 273 = 350K
and the pressure from mmHg to atm
623 mmHg . 1 atm/760 mmHg = 0.82 atm
We replace data: 0.82 atm . 17.5L = n . 0.082 L.atm/mol.K . 350K
(0.82 atm . 17.5L) / (0.082 L.atm/mol.K . 350K) = n
0.50 moles = n
These are the moles that corresponds to 22 g of the gas, so the molar mass will be → 22g / 0.50 mol = 44 g/mol
That molar mass corresponds to CO₂ → 12 g (C) + 16 g (O) . 2 = 44 g/mol
D. 2- youre adding two negative charges to a neutral element
Answer:
A.0.51L
B 1.67L
Explanation:
using the formula ;C1V1 =C2V2
15.8×V1=2×4
15.8V1=8
V1=8/15.8
V1=0.51L
apply the same method for B
