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Viktor [21]
3 years ago
14

A 1000-W iron is left on the ironing board with its base exposed to the air at 23◦C. The convection heat transfer coefficient be

tween the base surface and the surrounding air is 20W/(m2◦C). If the base has an emissivity of 0.4 and a surface area of 0.02m2, determine the temperature of the base of the iron.

Chemistry
1 answer:
Xelga [282]3 years ago
5 0

Answer:

216.52°C

Explanation:

Hi,  in this problem we know the total heat transfer is 1000 W.

We need to do know is the surface temperature of the iron.

So we are going to use the equation for radiation heat transfer.

 So, we have the next data

A = 0.02 m^2

ε= 0.4

h = 20 W/m2·°C

T_∞ = 20°C.  

We can assume that the air temperature is Tsurfaces = 20°C = 293.15 K.  The Stefan-Boltzmann constant, σ = 5.670x10-8 W/m^2·K^4.  

Remember that we have to use Kelvin temperatures for the convection term

Q=100W=A[h(Tiron-Tinfinity)+epsilon*Boltzmann(T^4iron-T^4surface)]

[Q=100W=(0.02m^2)[20\frac{W}{m^2C} (T_(iron)-296.15K))+0.4*5.670x10^-8(T^4iron-(296.15)^4)]=489.674

489.674K⇒216.52°C

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pishuonlain [190]

Answer:

50

Explanation:

We will need a balanced equation with masses, moles, and molar masses of the compounds involved.

1. Gather all the information in one place with molar masses above the formulas and masses below them.  

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               2NO   +   O₂ ⟶ 2NO₂

Mass/g:  80.00     16.00

2. Calculate the moles of each reactant  

\text{moles of NO} = \text{80.00 g NO} \times \dfrac{\text{1 mol NO}}{\text{30.01 g NO}} = \text{2.666 mol NO}\\\\\text{moles of O}_{2} = \text{16.00 g O}_{2} \times \dfrac{\text{1 mol O}_{2}}{\text{32.00 g O}_{2}} = \text{0.5000 mol O}_{2}

3. Calculate the moles of NO₂ we can obtain from each reactant

From NO:

The molar ratio is 2 mol NO₂:2 mol NO

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From O₂:

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\text{Moles of NO}_{2} =  \text{0.5000 mol O}_{2}\times \dfrac{\text{2 mol NO}_{2}}{\text{1 mol Cl}_{2}} = \text{1.000 mol NO}_{2}

4. Identify the limiting and excess reactants

The limiting reactant is O₂ because it gives the smaller amount of NO₂.

The excess reactant is NO.

5. Mass of excess reactant

(a) Moles of NO reacted

The molar ratio is 2 mol NO:1 mol O₂

\text{Moles reacted} = \text{0.500 mol O}_{2} \times \dfrac{\text{2 mol NO}}{\text{1 mol O}_{2}} = \text{1.000 mol NO}

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(c) Mass of NO remaining

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The answer should be:

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4 years ago
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