Answer:
B) The cold air moves faster and pushes the warm air away, causing condensation and rain.
decameters - meters: multiply by 10
meters to meters: multiply by 1
centimeters to meters: divide by 100
millimeters to meters: divide by 1000
For the rows at the bottom:
hectometer row: 100, multiply by 100, 4500
decameter row: 10, multiply by 10, 450
meter row: 1, multiply by 1, 45
decimeter row: 0.1, divide by 10, 4.5
centimeter row: 0.01, divide by 100, 0.45
im guessing theres a millimeter row at the bottom:
millimeter row: 0.001, divide by 1000, 0.045
hope this helps!
Answer:
Mass of Fe produced = 3.86785211069 ≈ 3.87 kg
Explanation:
From the question the chemical reaction can be written as follow :
Fe2O3 + C → Fe + CO
Balance the equation
Fe2O3 + 3C → 2Fe + 3CO
compute the molecular mass of Fe2O3 and atomic mass of Iron(Fe)
Molecular mass of Fe2O3 = 55.845(2) + 15.999(3) = 111.69 + 47.997 = 159.687 g
Atomic mass of iron = 55.845 g
From the balanced equation
159.687 g of Fe2O3 produces 2 × 55.845 = 111.69 g of Fe(iron)
Convert the 5.53 kg to gram
1 kg = 1000 g
5.53 kg = 5.53 × 1000 = 5530 g
since,
159.687 g of Fe2O3 produces 2 × 55.845 = 111.69 g of Iron(Fe)
5530 g of Fe2O3 will produce
cross multiply
Mass of Fe produced =5530 × 111.69/159.687
Mass of Fe produced = 617645.7
/159.687
Mass of Fe produced = 3867.85211069 g
convert to kg
1000 g = 1 kg
3867.85211069 = 3867.85211069/1000
Mass of Fe produced = 3.86785211069 ≈ 3.87 kg
<u>Answer:</u> The 
of the reaction at given temperature is -12.964 kJ/mol.
<u>Explanation:</u>
For the given chemical reaction:
The expression of 
for the given reaction:
We are given:
Putting values in above equation, we get:
To calculate the Gibbs free energy of the reaction, we use the equation:
where,
= Gibbs' free energy of the reaction = ?
= Standard gibbs' free energy change of the reaction = 0 J (at equilibrium)
R = Gas constant = 
T = Temperature = ![25^oC=[25+273]K=298K](https://tex.z-dn.net/?f=25%5EoC%3D%5B25%2B273%5DK%3D298K)
= equilibrium constant in terms of partial pressure = 
Putting values in above equation, we get:
Hence, the of the reaction at given temperature is -12.964 kJ/mol.
Answer:
Final temperature = T₂ = 155.43 °C
Explanation:
Specific heat capacity:
It is the amount of heat required to raise the temperature of one gram of substance by one degree.
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
Given data:
Mass of coin = 4.50 g
Heat absorbed = 54 cal
Initial temperature = 25 °C
Specific heat of copper = 0.092 cal/g °C
Final temperature = ?
Solution:
Q = m.c. ΔT
ΔT = T₂ -T₁
Q = m.c. T₂ -T₁
54 cal = 4.50 g × 0.092 cal/g °C × T₂ -25 °C
54 cal = 0.414 cal/ °C × T₂ -25 °C
54 cal /0.414 cal/ °C = T₂ -25 °C
130.43 °C = T₂ -25 °C
130.43 °C + 25 °C = T₂
155.43 °C = T₂
