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Keith_Richards [23]
3 years ago
12

How much heat is absorbed by a 56g iron skillet when its temperature rises from 15oC to 27oC?

Chemistry
1 answer:
wel3 years ago
4 0

we know that Q=mc_{p}ΔT

m=56g

°T_{1} =15°C

T_{2} =27°C

Q=56*0.450*(27-15)=302.4J

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I’m assuming the top ruler has more measurement points, like more specific numbers. This would mean the top ruler is more reliable because you can be more specific with your measurements
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What is an emission spectrum?
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The reform reaction between steam and gaseous methane (CH4) produces "synthesis gas," a mixture of carbon monoxide gas and dihyd
kenny6666 [7]

Answer:

The answer is "= 0.078 \ kg \ H_2".

Explanation:

calculating the moles in CH_4 =\frac{PV}{RT}

                                                =\frac{(0.58 \ atm) \times (923 \ L) }{ (0.0821 \frac{L \cdot atm}{K \cdot mol})(232^{\circ} C +273)}\\\\=\frac{(535.34 \ atm \cdot \ L) }{ (0.0821 \frac{L \cdot atm}{K \cdot mol})(505)K}\\\\=\frac{(535.34 \ atm \cdot \ L) }{ (41.4605 \frac{L \cdot atm}{mol})}\\\\= 12.9 \ mol

Eqution:

CH_4 +H_2O \to  3H_2+ CO \ (g)

Calculating the amount of H_2 produced:

= 12.9 \ mol CH_4 \times  \frac{3 \ mol \ H_2 }{1 \ mol \ CH_4}\times \frac{2.016 g H_2}{1 \ mol \ H_2}\\\\= 78 \ g \ H_2 \\\\= 0.078 \ kg \ H_2

So, the amount of dihydrogen produced = 0.078 \frac{kg}{s}

5 0
3 years ago
An atom of which of these elements most likely forms an anion? A. AI B. Br C. Ca D. Mg
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3 years ago
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When butane burns completely, only water and carbon dioxide gas are produced. If 11.6 g of butane and 40.0 L of oxygen at 22.0o
Angelina_Jolie [31]

19.7 litre volume of carbon dioxide gas at 22.0o C and 102 kPa can be collected over water.

<h3>What is vapour pressure?</h3>

Vapour pressure is a measure of the tendency of a material to change into the gaseous or vapour state, and it increases with temperature.

Moles of Butane = mass in grams / molar mass = 11.6 / 58.12 = 0.2

Volume of O_2 (V) = 40 liter

Temperature (T) = 22°C = 22 + 273 = 295 K

Pressure (P) = 102 kPa = 102 / 101.325 = 1.007 atm

Moles of O_2 (n) can be calculated by ideal gas equation.

PV = nRT

n = 1.007 40 ÷ 0.0821 295 = 1.663

Balanced chemical reaction;

2C_4H_10 + 13O_2 ---> 8CO_2 + 10H_2O

From reaction;

13 moles O_2 require 2 moles C_4H_10

So, 1.663 moles O_2 will require = 2 x 1.663 ÷13 = 0.256 moles of C_4H_10

Thus C_4H_10 is a limiting reagent. So it will drive the yield of CO_2.

Moles of CO_2 produced = (8/2) 0.2 = 0.8 moles

Pressure of CO_2 (P) = 102 - 2.24 = 99.76 kPa = 99.76  ÷ 101.325 = 0.985 atm

Applying the ideal gas equation for CO_2,

PV = nRT

0.985 V = 0.8 0.0821 x 295

V = 19.7 liter

The volume of CO_2 produced = 19.7 liter.

Learn more about the vapour pressure here:

brainly.com/question/25699778

#SPJ1

5 0
2 years ago
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