Answer:
1.03 atm
Explanation:
Primero <u>convertimos 21 °C y 37 °C a K</u>:
- 21 °C + 273.16 = 294.16 K
- 37 °C + 273.16 = 310.16 K
Una vez tenemos las temperaturas absolutas, podemos resolver este problema usando la<em> ley de Gay-Lussac</em>:
En este caso:
Colocando los datos:
- 294.16 K * P₂ = 310.16 K * 0.98 atm
Y <u>despejando P₂</u>:
Answer: -
O 2 limiting reagent
53.83 g CO2 theoretical Yield
97.9% percentage yield
Explanation: -
Mas of CH4 = 23.2 g
Molar mass of CH4 = 12 x 1 + 1 x 4 = 16g
Mass of O2 = 78.3 g
Molar mass of O 2 – 16 x 2 = 32 g
The balanced chemical equation for the reaction is
CH4 + 2 O2 = CO2 + 2 H2O
From the balanced equation we see that
2 O 2 reacts with 1 CH4
2 x 32 g of O 2 react with 16 g of CH4
78.3 g of O 2 react with

= 19.575 g pf CH4
Thus CH4 is in excess.
The limiting reagent is thus O 2.
Molar mass of CO2 = 12 x 1 + 16 x 2= 12 +32 = 44g
From the balanced equation we see
2O 2 gives 1 CO2
2 x 32 g of O 2 gives 44g of CO2
78.3 g of O 2 gives =

=53.83 g of CO2
Theoritical Yield = 53.83 g of CO2
Actual yield = 52.7 g
Percentage yield =

=97.9 %
Answer:
new solubility = 0.443 g/l
Explanation:
To solve this question, we will use Henry's law.
Henry's law states that, at constant temperature:
S1 / P1 = S2 / P2
We are given that:
S1 = 0.16 g/l
P1 = 104 kPa
S2 is the solubility we want to calculate
P2 = 288 kPa
Substitute with the givens in the above relation to get the new solubility (S2) as follows:
0.16 / 104 = S2 / 288
S2 = (0.16/104) * 288
S2 = 0.443 g/l
Hope this helps :)