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1 year ago

How many neutrons does an atom of Uranium 240?

Chemistry

1 answer:

qwelly [4]1 year ago

4 0

Answer:

Number of neutrons is equal to 148.

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Using the equation MgCl2 -> Mg + Cl2, if 5.00 grams of MgCl2 is given, how many grams of Mg is produced?

motikmotik

Answer:

MgCl2-> Mg+Cl

mass 5.00g Mass=1.263g

RFM Mg=24+35.5 ×2= 95 RFM= 24

moles= 5.00÷ 95= 0.0526 Moles=0.0526

Explanation:

mas of Mg= 1.263 grams

4 0

3 years ago

Using the molarity equation, calculate how many grams of salt you need in order to make 80ml of a 2M solution (MW = 58.44g/mole)

ollegr [7]

Answer:

9.35g

Explanation:

The molarity equation establishes that:

$\textrm{molarity}=\frac{\textrm{moles of solute}}{\textrm{liters of solution}}$

So, we have information about molarity (2M) and volume (80 ml=0.08 l), with that, we can find the moles of solute:

$\textrm{moles of solute}=\textrm{molarity}*\textrm{liters of solution}$

$\textrm{moles of solute}= 0.08 \textrm{ l} *2\textrm{ M} = 0.16 \textrm{ mol}$

The mathematical equation that establishes the relationship between molar weight, mass and moles is:

$\textrm{molar weight}= \frac{\textrm{mass}}{\textrm{moles}}$

$\textrm{MW}= \frac{\textrm{m}}{\textrm{n}}$

We have MW (58.44g/mole) and n (0.16 mol), and we need to find m (grams of salt needed) to solve the problem:

$\textrm{m} = \textrm{MW * n}= 58.44\frac{\textrm{g}}{\textrm{mol}} * 0.16 \textrm{ mol} = 9.35 \textrm{ g}$

8 0

3 years ago

Of the following: H2(g); He(g); CO2(g); which would behave least like an ideal gas? Why?

Margarita [4]

Answer:

CO2(g)

Because CO2 is the larges molecule with specific geometric, therefore it is not likely to behave as an ideal gas.

4 0

3 years ago

Which of the following describes the greenhouse effect?

forsale [732]

Answer:

Explanation:

Earth's greenhouse gases trap heat in the atmosphere and warm the planet.

5 0

3 years ago

Which conversion factor do you use first to calculate the number of grams of CO 2 produced by the reaction of 50.6 g of CH 4 wit

Brilliant_brown [7]

Answer:

Thus, first conversion of mass of methane into moles by dividing it with 16.04 g/mol

Mass = 138.63 g

Explanation:

The balanced chemical reaction is shown below:-

$CH_4+2O_2\rightarrow CO_2+2H_2O$

Firstly the moles of methane gas reacted must be calculate as:-

Given, mass of methane = 50.6 g

Molar mass of methane gas = 16.04 g/mol

The formula for the calculation of moles is:-

$Moles=\frac{Mass\ taken}{Molar\ mass}=\frac{50.6}{16.04}\ mol=3.15\ mol$

Thus, from the reaction stoichiometry,

1 mole of methane produces 1 mole of carbon dioxide

Also,

3.15 mole of methane produces 3.15 mole of carbon dioxide

Moles of $CO_2$ = 3.15 mole

Molar mass of $CO_2$ = 44.01 g/mol

Mass = Moles*Molar mass = $3.15\times 44.01$ g = 138.63 g

3 0

3 years ago