Answer:
165 of CO₂.
Explanation:
In the reaction:
Na2CO3 + 2HCl → 2NaCl + CO2 + H2O
2 moles of HCl reacts producing 1 mole o CO₂
If 7.5 moles of HCl reacts, moles of CO₂ produced are:
7.5 moles of HCl ₓ ( 1 mol CO₂ / 2 mol HCl) = 3.75 mol CO₂. As molar mass of CO₂ is 44g/mol, mass of CO₂ is:
3.75 mol CO₂ ₓ (44g / 1mol) = <em>165 of CO₂ </em>
To allow for equations and problems in chemistry to be as precise as possible. When experiments are conducted, and even if the number is the slightest bit off, the problem or experiment could be impacted very negatively. It allows for complete accuracy to ensure nothing goes wrong, since chemistry is very touchy and risky when dealing with extremely unsafe elements.
Answer:
Pressure = 1.14 atm
Explanation:
Hello,
This question requires us to calculate the final pressure of the bottle after thermal equilibrium.
This is a direct application of pressure law which states that in a fixed mass of gas, the pressure of a given gas is directly proportional to its temperature, provided that volume remains constant.
Mathematically, what this implies is
P = kT k = P / T
P1 / T1 = P2 / T2 = P3 / T3 =........= Pn / Tn
P1 / T1 = P2 / T2
P1 = 1.0atm
T1 = -15°C = (-15 + 273.15)K = 258.15K
P2 = ?
T2 = 21.5°C = (21.5 + 273.15)K = 294.65K
P1 / T1 = P2 / T2
P2 = (P1 × T2) / T1
P2 = (1.0 × 294.65) / 258.15
P2 = 1.14atm
The pressure of the gas after attaining equilibrium is 1.14atm
amount of product formed or amount of reactants used / time
