Answer:
1 = Q = 7315 j
2 =Q = -21937.5 j
Explanation:
Given data:
Mass of water = 50 g
Initial temperature = 20°C
Final temperature = 55°C
Energy required to change the temperature = ?
Solution:
Specific heat capacity:
It is the amount of heat required to raise the temperature of one gram of substance by one degree.
Specific heat capacity of water is 4.18 j/g.°C.
Formula:
Q = m.c. ΔT
Q = amount of heat absorbed or released
m = mass of given substance
c = specific heat capacity of substance
ΔT = change in temperature
ΔT = T2 - T1
ΔT = 55°C - 20°C
ΔT = 35°C
Q = 50 g× 4.18 j/g.°C×35°C
Q = 7315 j
Q 2:
Given data:
Mass of metal = 100 g
Initial temperature = 1000°C
Final temperature = 25°C
Energy released = ?
Specific heat capacity = 0.225 j/g.°C
Solution:
Q = m.c. ΔT
Q = amount of heat absorbed or released
m = mass of given substance
c = specific heat capacity of substance
ΔT = change in temperature
ΔT = T2 - T1
ΔT = 25°C - 1000°C
ΔT = -975°C
Now we will put the values in formula.
Q = 100 g × 0.225 j/g.°C × -975°C
Q = -21937.5 j
Negative sign show that energy is released.
Given:
n = 12 moles of oxygen
T = 273 K, temperature
p = 75 kPa, pressure
Use the ideal gas law, given by
where
V = volume
R = 8.3145 J/(mol-K), the gas constant
Therefore,
Answer: 0.363 m³
Answer:
I2 + 2S2O3^2- --------> S4O6^2- + 2I^-
Explanation:
The correct equation is;
2Na2S2O3 + I2 → Na2S4O6 + 2NaI
Oxidation half equation;
2S2O3^2- --------> S4O6^2- + 2e-
Reduction half equation;
I2 + 2e ----------> 2I^-
Overall balanced redox reaction equation;
I2 + 2S2O3^2- --------> S4O6^2- + 2I^-
Is this just free points or is there a question
To convert on unit to another unit, a conversion factor is needed to multiply in the value given. For the value given above, we have to convert it from miles per gallon to kilometers per liter. The factors to be used are:
1 mile = 1.61 kilometers;
1 gallon = 3.79 liters.
<span>34.0 miles / gallon ( 1.61 kilometers / 1 mile ) ( 1 gallon / 3.79 L ) = 14.44 kilometer / liter</span>
