Answer:
Mass = 713.4 ×10⁻⁴ g
Explanation:
Given data:
Number of moles of calcium phosphate = 2.3×10⁻⁴ mol
Mass of calcium phosphate = ?
Solution:
Formula:
Number of moles = mass/molar mass
Molar mass of calcium phosphate is 310.18 g/mol
by putting values,
2.3×10⁻⁴ mol = mass / 310.18 g/mol
Mass = 2.3×10⁻⁴ mol × 310.18 g/mol
Mass = 713.4 ×10⁻⁴ g
pressure increases as depth increases.
Answer:
328.4KJ
Explanation:
Before we move on to calculate enthalpy change, we calculate the amount of heat Q
Q= mcΔT
m = density * volume = 250 * 1.25 = 312.5g
c = 3.74J/g.k
ΔT = 7.80 + 273.15K = 280.95K
Q= 312.5 * 3.74 * 280.95 = 328,360.312 J= 328.4KJ(1000J = 1KJ, so divide by 1000)
The enthalpy change in the reaction is same as amount of heat transferred = 328.4KJ
Answer:
In an equilibrium mixture of the three gases, PCO = PCl2 = 2.22 × 10-4 atm. The partial pressure of the product, phosgene (COCl2), is kp=(COCl2)/(CO)(Cl2) which is . So, the correct answer is 7.34.
