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2 years ago

Which statement is true about word equations with regards to chemical reactions?

Chemistry

1 answer:

Akimi4 [234]2 years ago

6 0

The total mass of the reactants equals the total mass of the products

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What is the mass of 0.1 mole of Cu(OH) 2 ?

Citrus2011 [14]

Answer:

0.1

Explanation:

I know that because of the law of conservation of mass

7 0

3 years ago

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When considering the relationship among standard free energy change, equilibrium constants, and standard cell potential, the equ

DedPeter [7]

Answer:

ΔG° = - RTLnK is used to find the standard cell potential given the equilibrium constant

Explanation:

for an ideal disolution:

⇒ ΔG = RT∑ni LnXi

∴ ΔG = ( μi - μi*)ni

∴ μ : chemical potential

∴ μ*: chem. potential of the pure component at T and P.

⇒ ΔG = μi - μi* = RT LnXi

for a equilibrium reaction:

⇒ ∑ νi*μi = 0

⇒ ΔGr = ΔG°+ RT Ln Kx = 0

⇒ ΔG° = - RT LnKx

4 0

4 years ago

Attem A liquid solvent is added to a flask containing an insoluble solid. The total volume of the solid and liquid together is 9

monitta

Answer: The mass of solid is 105.4 g

Explanation:

To calculate the density of a substance, we use the equation"

$\text{Density of a substance}=\frac{\text{Mass of a substance}}{\text{Volume of a substance}}$ .......(1)

For liquid:

Mass of liquid = 26.6 g

Density of liquid = 0.865 g/mL

Putting values in equation 1, we get:

$0.865g/mL=\frac{26.6g}{\text{Volume of liquid}}\\\\\text{Volume of liquid}=\frac{26.6g}{0.865g/mL}=30.8mL$

We are given:

Volume of solid + Volume of liquid = 91.0 mL

Volume of liquid = 30.8 mL

So, volume of solid = 91.0 - 30.8 = 60.2 mL

Now, calculating the mass of solid by using equation 1, we get:

Volume of solid = 60.2 mL

Density of solid = 1.75 g/mL

Putting values in equation 1, we get:

$1.75g/mL=\frac{\text{Mass of solid}}{60.2mL}\\\\\text{Mass of solid}=(1.75g/mL\times 60.2mL)=105.4g$

Hence, the mass of solid is 105.4 grams

7 0

3 years ago

Write the balanced equation for the reaction given below: C2H6 + O2 --> CO2 + H2O. If 16.4 L of C2H6 reacts with 0.980 mol of

Natalka [10]

The balanced reaction: C2H6 + 7/2 O2 -> 2 CO2 + 3 H2O

We first convert volume of C2H6 to no. of moles. We use the conditions at STP where 1 mol = 22.4 L thus,

Moles C2H6 = 16.4 L/ 22.4 L =0.7321 mol

In order to determine the limiting reagent, we look at the given amounts of the reactants.

0.7321 mol C2H6 (7/2 mol O2 / 1 mol C2H6) = 2.562 mol O2

From the given amounts of the reactants, we can say that O2 is the limiting reactant since we need 2.562 mol O2 to completely react the given amount of C2H6. The excess reagent is C2H6

To calculate for the amount of products and excess reactants:

0.980 mol O2 (2 mol CO2 / (7/2 mol O2)) = 0.56 mol CO2 (22.4 L / 1 mol ) =12.544 L CO2
0.980 mol O2 (1 mol C2H6 / (7/2 mol O2)) = 0.28 mol C2H6
Excess C2H6 = 0.7321 mol - 0.28 mol C2H6 = 0.4521 mol C2H6

We then use the molecular weight of C2H6 to convert the excess amount to grams.

0.4521 mol C2H6 (30.08 g C2H6 / 1 mol C2H6) = 13.60 g C2H6

Since the limiting reagent is O2 there will be no oxygen atoms that will be left after the reaction.

5 0

3 years ago

This is for my science class.

Kay [80]

Answer:

4 joules

Hope this helps if it does consider giving brainliest

Cya on the next one!

Explanation:

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3 years ago

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