Answer:
D
Explanation:
The sample must contain impurity that is lower in atomic mass to sodium and since potassium has higher atomic mass to sodium, the answer is the sample contains NaCl and LiCl. We are sure already that the sample is not pure which rules out option a and option b contains sodium iodide which cannot contribute to the increase in chlorine
Answer:
Mass = 7.2 g
Explanation:
Given data:
Mass of water produced = ?
Mass of oxygen = 7.8 g
Solution:
Chemical equation:
2H₂ + O₂ → 2H₂O
Number of moles of oxygen:
Number of moles = mass/ molar mass
Number of moles = 7.8 g/ 32 g/mol
Number of moles = 0.2 mol
Now we will compare the moles of water with oxygen.
O₂ : H₂O
1 : 2
0.2 : 2×0.2 = 0.4 mol
Mass of water:
Mass = number of moles × number of moles
Mass = 0.4 mol × 18 g/mol
Mass = 7.2 g
Answer: 
.
Explanation:
Temperature of the gas is defined as the degree of hotness or coldness of a body. It is expressed in units like 
and 
These units of temperature are inter convertible.
We are given:
Temperature of the gas = 
(1mK=0.001 K)
Converting this unit of temperature into by using conversion factor:
Thus 
Thus the temperature is .
What is the amount of heat, in joules, required to increase the temperature of a 49.5-gram sample of water from 22°C to 66°C?
- (1) 9100 J
- (2) 4600 J
- (3) 1400 J
- (4) 2300 J
<u>Answer:</u>
9100 J is the amount of heat, in joules, required to increase the temperature of a 49.5-gram sample of water from 22°C to 66°C.
<u>Explanation:</u>
Given: Q = ? J
mass = 49.5 g = 0.0495 kg
T1 = 22°C
T2 = 66°C
Cp = 4.18 J/Kg°C
Q = mCpΔT
Q = (4.95)(4.18)(66 - 22)
Q = 9104 J
So 9100 J is the amount of heat, in joules, required to increase the temperature of a 49.5-gram sample of water from 22°C to 66°C.
