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3 years ago

using the symbol M for the element, write the chemical formula for the compound that forms when element M reacts with iodine.

Chemistry

2 answers:

Anon25 [30]3 years ago

6 0

Answer : The chemical formula for the compound is, $MI$

Explanation :

When the element 'M' react with the $I_2$ to give $MI$ .

The balanced chemical reaction is,

$2M+I_2\rightarrow 2MI$

In this reaction, 'M' is in mono-atomic form and $I_2$ is in diatomic form.

By the stoichiometry,

2 moles 'M' react with the 1 mole of $I_2$ to give 2 moles of $MI$ .

Therefore, the chemical formula of the compound is, $MI$

KIM [24]3 years ago

3 0

When the element M connects with Iodine and it attracts a postive reaction which will give you a formula of M+i=iodine

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3 years ago

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Tanya [424]

Answer:

$V=23.9mL$

Explanation:

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In this case for the solution you are given, we first use the mass to compute the moles of CuNO3:

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2 years ago

Define the law of conservation of charge and provide an example.

iren2701 [21]

Answer:

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3 years ago

You have 4 moles of oxygen gas in a flask. 4 moles of helium gas is added. What happens to the total pressure of the gases in th

ASHA 777 [7]

Answer: The correct option is (c). The total pressure doubles.

Solution:

Initially, only 4 moles of oxygen gas were present in the flask.

$p_{O_2}=Tp_1\times X_{O_2}$ ( $X_{O_2}=\frac{4}{4}$ ) ( according to Dalton's law of partial pressure)

$p_{O_2}=Tp_1\times 1=Tp_1$ ....(1)

$Tp_1$ = Total pressure when only oxygen gas was present.

Final total pressure when 4 moles of helium gas were added:

$X'_{O_2}=\frac{4}{8}=\farc{1}{2},X_{He}=\frac{4}{8}=\frac{1}{2}$

partial pressure of oxygen in the mixture :

Since, the number of moles of oxygen remains the same, the partial pressure of oxygen will also remain the same in the mixture.

$p_{O_2}=Tp_2\times X'_{O_2}=Tp_2\times \frac{1}{2}$

$Tp_2$ = Total pressure of the mixture.

from (1)

$Tp_1=Tp_2\times X'_{O_2}=Tp_2\times \frac{1}{2}$

On rearranging, we get:

$Tp_2=2\times Tp_1$

The new total pressure will be twice of initial total pressure.

7 0

2 years ago

A sample of gas has a mass of 0.560 g . Its volume is 125 mL at a temperature of 85 ∘C and a pressure of 757 mmHg .

-BARSIC- [3]

Answer:

132g/mole

Explanation:

using the formula PV=nRT should be used to solve for the number of moles (n). R is a constant which is 62.3637 L mmHG/mole K.

Inorder for your units to match you will have to convert 125ml to .125L and the temperature of 85C to K . you do that by adding 273 to the 85C and get 358K. Once you solve for n then you use that number and divide by the number of grams from the question (.560g) since molar mass is grams/moles.

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3 years ago