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2 years ago

12

identify the law that explains the following observation nitrogen dioxide can be formed by reacting 14 G of nitrogen with 32 gra

ms of oxygen

1 answer:

Mrrafil [7]2 years ago

8 0

Answer:

The law of definite proportions. I had the same question for chemistry and this is what they said was right so I got 100%.

Explanation:

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If the mass of a material is 91 grams and the volume of the material is 20 cm3, what would the density of the material be?

AlekseyPX

Use the formula Density=Mass/Volume

8 0

3 years ago

3. A 31.2-g piece of silver (s = 0.237 J/(g · °C)), initially at 277.2°C, is added to 185.8 g of a liquid, initially at 24.4°C,

VARVARA [1.3K]

Answer:

$Cp_{liquid}=2.54\frac{J}{g\°C}$

Explanation:

Hello,

In this case, since silver is initially hot as it cools down, the heat it loses is gained by the liquid, which can be thermodynamically represented by:

$Q_{Ag}=-Q_{liquid}$

That in terms of the heat capacities, masses and temperature changes turns out:

$m_{Ag}Cp_{Ag}(T_2-T_{Ag})=-m_{liquid}Cp_{liquid}(T_2-T_{liquid})$

Since no phase change is happening. Thus, solving for the heat capacity of the liquid we obtain:

$Cp_{liquid}=\frac{m_{Ag}Cp_{Ag}(T_2-T_{Ag})}{-m_{liquid}(T_2-T_{liquid})} \\\\Cp_{liquid}=\frac{31.2g*0.237\frac{J}{g\°C}*(28.3-227.2)\°C}{185.8g*(28.3-24.4)\°C}\\ \\Cp_{liquid}=2.54\frac{J}{g\°C}$

Best regards.

6 0

3 years ago

B) How many kilojoules of heat will be released by the combustion of 22.52 g of this liquid at

snow_tiger [21]

Answer:

Explanation:

You realize that C2H5OH releases -1277.3kJ/mol. We need to convert this to the amount based on the question. We that 22.52g of C2H5OH = 0.48884 mol.

This means that it will release (-1277.3)(0.48884) = 624.40 KJ of heat will be released. Note the negative sign is not necessary here (I think) because it says how much is released and not the change in heat of the system so it should be positive.

3 0

2 years ago

PLZ HELP QUICK!!

MissTica

I have the same question too!!!Dang I thought I would get a answer I just guessed

8 0

2 years ago

1. 17.0 grams of xenon hexafluoride is in a solid container. How many milliliters of that gas

BlackZzzverrR [31]

Answer: The volume of gas is 3020 ml

Explanation:

According to ideal gas equation:

$PV=nRT$

P = pressure of gas = 821.4 torr = 1.08 atm (760 torr = 1atm)

V = Volume of gas in L = ?

n = number of moles = $\frac{\text {given mass}}{\text {Molar mass}}=\frac{17.0g}{245.28g/mol}=0.069mol$

R = gas constant = $0.0821Latm/Kmol$

T =temperature = $302.7^0C=(302.7+273)K=575.7K$

$V=\frac{nRT}{P}$

$V=\frac{0.069mol\times 0.0821Latm/K mol\times 575.7K}{1.08atm}=3.02L=3020ml$

Thus volume of gas is 3020 ml

4 0

2 years ago