A...because both of them(carbon and oxygen)are nonmetal
Answer : The partial pressure of nitrogen gas is, 2.94 atm
Explanation:
According top the Henry's Law, the concentration of a gas in a liquid is directly proportional to the partial pressure of the gas.
is Henry's constant.
or,
where,
= initial concentration of gas = 
= final concentration of gas = 
= initial partial pressure of gas = 0.78 atm
= final partial pressure of gas = ?
Now put all the given values in the above formula, we get the final partial pressure of the gas.
Therefore, the partial pressure of nitrogen gas is, 2.94 atm
Answer:
K = 351.3
Explanation:
The relationship between the Celsius scale and kelvin scale is;
K = 273 + C
Since the Celsius temperature = 78.3
The kelvin temperature is given as;
K = 273 + 78.3
K = 351.3
from ICE table
H2(g) + I2 (g )↔ 2HI(g)
equ 0.958 0.877 0.02 first mix1
0.621 0.621 0.101 sec mix2
Kp1 = P(HI)^2 / p(H2)*p(I2) for mix 1
= 0.02^2 / 0.958*0.877
= 4.8x10^-4
Kp2 = P(HI)^2 / P(H2)* P(I2) for mix 2
= 0.101^2/ 0.621*0.621
= 0.0265
we can see that Kp1< Kp2 that means that the sec mixture is not at equilibrium. It will go left to reduce its products and increase reactant to reduce the Kp value to achieve equilibrium.
and the partial pressure of Hi when mix 2 reach equilibrium is:
4.8x10^-4 = P(Hi)^2 / (0.621*0.621)
∴ P(Hi) at equilibrium = 0.0136 atm
2 C2H6 + 7 O2 -> 4CO2 + 6 H2O
<span>so the products are carbondioxide & water vapour</span>
