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GREYUIT [131]
3 years ago
8

According to the ideal gas law for a fixed amount of gas, if the _____ is constant, then when the ________ increases the volume

should ________.
a) temperature, pressure, increase
b) pressure, temperature, decrease
c) pressure, volume, decrease
d) none of the above
Chemistry
1 answer:
BARSIC [14]3 years ago
5 0

Answer:

D. none of the above

Explanation:

A. is wrong because pressure and volume have an inverse relationship. When one increases the other decreases, this is not an option.

B. is wrong because temperature and volume have a proportional relationship. One one goes up, the other goes up or vice versa.

C. is wrong because volume cannot increase the then decrease at the same time.

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What is the mass in grams of a 8.4 mole sample of iron?
wlad13 [49]
8.4 moles equals 469.14g Fe
5 0
3 years ago
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Calculate the mass of chromium metal produced when 425.0mL of 0.25M chromium(ll) nitrate reacts with a strip of zinc that remain
Reil [10]

The balanced chemical equation for the production of chromium metal from the reaction of chromium(ll) nitrate reacts with a strip of zinc is:

3 Zn + 2 Cr(NO₃)₃ → 2 Cr + 3 Zn(NO₃)₂

This is a redox reaction, which <u>is a chemical reaction in which one or more electrons are transferred between the reagents</u>, causing a change in their oxidation states. In the proposed reaction, Cr oxidation state goes from +3 to 0, becoming metallic chromium, while Zn goes from being Zn⁰ to Zn²⁺.

<u>The mass of chromium metal produced in the above reaction will be,</u>

425.0 mL x \frac{1 L}{1000 mL} x  \frac{0.25 mol Cr(NO_{3})_{3}  }{1 L} x \frac{2 mol Cr  }{2 mol Cr(NO_{3})_{3} } x \frac{51.9961 g Cr}{1 mol Cr} = 5.52 g

So, the mass of chromium metal produced when 425.0mL of 0.25M chromium(ll) nitrate reacts with a strip of zinc that remains in excess is 5.52 g of Cr.

6 0
3 years ago
Nitrogen gas (112 g) reacts with hydrogen gas to produce 40.8 g of ammonia according to the following
Lemur [1.5K]

Answer:

%yield of NH₃ = 30%

Explanation:

Actual yield of NH₃ = 40.8g

Theoretical yield = ?

Equation of reaction

N₂ + 3H₂ → 2NH₃

Molar mass of NH₃ = 17g/mol

Molarmass of N = 14.00

2 molecules of N = 2 * 14.00 = 28g/mol

Number of moles = mass / molar mass

Mass = number of moles * molar mass

Mass = 1 * 28.00 = 28g of N₂ (the number of moles of N₂ from the equation is 1).

From the equation of reaction,

28g of N₂ produce (2 * 17)g of NH₃

28g of N₂ = 34g of NH₃

112g of N₂ = x g of NH₃

X = (112 * 34) / 28

X = 136g of NH₃

Theoretical yield = 136g of NH₃

% yield = (actual yield / theoretical yield) * 100

% yield = (40.8 / 136) * 100

% yield = 0.3 * 100

% yield = 30%

8 0
3 years ago
What does the number at the end of an element mean? (For example, Hydrogen-3)
Inga [223]

Answer:

The top number is the total mass number, particles in an atom of an element that have mass are protons and neutrons.

Explanation:

4 0
2 years ago
Is this right, i dont know how to do this?
aliina [53]
Your answer, I believe, is correct. I'm no expert at chemistry tho. 

Tyler Dewitt has some great YouTube vids on chem that have saved my butt on multiple occasions. you should check them out. very helpful
3 0
3 years ago
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