The partial pressure of oxygen is 4.84 atm, and the partial pressure of carbon dioxide is 4.37 atm.
Moles of O₂ = 52.5 g O₂ × (1 mol O₂/32.00 g O₂) = 1.641 mol O₂
Moles of CO₂ = 65.1 g CO₂ × (1 mol CO₂/44.01 g CO₂) = 1.479 mol CO₂
Total moles = (1.641 + 1.479) mol = 3.120 mol
Let<em> O₂ be Gas 1</em> and <em>CO₂ be Gas 2</em>.
χ₁= 1.641/3.120 = 0.5259
χ₂= 1.479/3.120 = 0.4741
<em>p</em>₁ = χ₁<em>p</em>_tot = 0.5259 × 9.21 atm = 4.84 atm
<em>p</em>₂ = χ₂<em>p</em>_tot = 0.4741 × 9.21 atm = 4.37 atm
To answer the question above, we make use of the equation,
heat = (specific heat ) x mass x (change in temperature)
Substituting the known values,
heat = (0.128 J/g°C) x (3.3 kg)(1000g / 1kg) x (69°C - 26°C)
= 18163.2 J
Therefore, the amount of heat required is approximately 18163.2 J.
When a system is in dynamic equilibrium, the forward reaction rate and the backward reaction rate are equal or occurs at the same rate. Therefore, the third option above is the most accurate one. Hope this answers the question. Have a nice day.
Answer:
FALSE
Explanation:
Keratinocytes begin to die in the stratum granulosum is False.
Answer:
5.67 g OF WATER WILL BE FORMED WHEN 13.7 g OF MnO2 REACTS WITH HCl GAS.
Explanation:
EQUATION FOR THE REACTION
Mn02 + 4HCl --------> MnCl2 + Cl2 + 2H2O
From the balanced reaction between manganese oxide and hydrogen chloride gas;
1 mole of MnO2 reacts to form 2 mole of water
At STP, the molecular mass of the sample is equal to the mole of the substance. So therefore:
(55 + 16 * 2) g of MnO2 reacts to form 2 * ( 1 *2 + 16) g of water
(55 + 32) g of MnO2 reacts to form 2 * 18 g of water
87 g of MnO2 reacts to form 36 g of water
If 13.7 g of MnO2 were to be used?
87 g of MnO2 = 36 g of H2O
13.7 g of MnO2 = ( 13.7 * 36 / 87) g of water
= 493.2 / 87 g of water
Mass of water = 5.669 g of water
Approximately 5.67 g of water will be formed when 13.7 g of manganese oxide reacts with excess hydrogen chloride gas.
