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3 years ago

If a gas occupies 79.5 mL at -1.4°C, what temperature, in Kelvin, would it

Chemistry

1 answer:

Anna35 [415]3 years ago

5 0

Answer:

121 K

Explanation:

Step 1: Given data

Initial volume (V₁): 79.5 mL

Initial temperature (T₁): -1.4°C

Final volume (V₂): 35.3 mL

Step 2: Convert "-1.4°C" to Kelvin

We will use the following expression.

K = °C + 273.15 = -1.4°C + 273.15 = 271.8 K

Step 3: Calculate the final temperature of the gas (T₂)

Assuming ideal behavior and constant pressure, we can calculate the final temperature of the gas using Charles' law.

V₁/T₁ = V₂/T₂

T₂ = V₂ × T₁/V₁

T₂ = 35.3 mL × 271.8 K/79.5 mL = 121 K

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Aqueous sulfuric acid will react with solid sodium hydroxide to produce aqueous sodium sulfate and liquid water . Suppose 6.9 g

satela [25.4K]

Answer:

$5.6gNa_2SO_4$

Explanation:

Hello,

In this case, the undergoing chemical reaction is:

$2NaOH(aq)+H_2SO_4(aq)\rightarrow Na_2SO_4(aq)+2H_2O(l)$

Therefore, since the masses of both of the reactants are given, one computes the available moles of sulfuric acid and those moles of it consumed by the sodium hydroxide as shown below:

$n_{H_2SO_4}^{available}=6.9gH_2SO_4*\frac{1molH_2SO_4}{98gH_2SO_4}=0.0704molH_2SO_4\\n_{H_2SO_4}^{consumed\ by\ NaOH}=3.14gNaOH*\frac{1molNaOH}{40gNaOH}*\frac{1molH_2SO_4}{2molNaOH}=0.04molH_2SO_4$

In such a way, since there is more available sulfuric acid than it that is consumed, the sodium hydroxide is the limiting reagent, consequently, the maximum mass of sodium sulfate turns out:

$m_{Na_2SO_4}=0.04molH_2SO_4*\frac{1molNa_2SO_4}{1molH_2SO_4} *\frac{142.04gNa_2SO_4}{1molNa_2SO_4}=5.6gNa_2SO_4$

Best regards.

5 0

3 years ago

Select the correct answer from each drop-down menu. An atom has 9 electrons and 9 protons at the start. If it loses 2 electrons,

aalyn [17]

Answer:

If it loses to electrons the net charge will be +2. If the atom instead gains 4 electrons, the net charge will be -4.

Explanation: When an atom loses electrons( which are negatively charged), it turns into a cation. This means since there is more protons(which are positively charged) than electrons, the charge is positive. The charge is positive and than the number of electrons lost. It is the exact opposite for gaining electrons.

3 0

3 years ago

Mass is usually measured using ?

Brut [27]

Balance
Usually it’s a triple beam balance.
A ruler measures length

8 0

2 years ago

Which coefficients will balance the following reaction:

valentina_108 [34]

Answer:

C ) 2, 1, 2

Explanation:

The given reaction is synthesis reaction in which lithium and bromine react to form lithium bromide.

Chemical equation:

Li + Br₂ → LiBr

Balanced chemical equation:

2Li + Br₂ → 2LiBr

Step 1:

Li + Br₂ → LiBr

left hand side Right hand side

Li = 1 Li = 1

Br = 2 Br = 1

Step 2:

Li + Br₂ → 2LiBr

left hand side Right hand side

Li = 1 Li = 2

Br = 2 Br = 2

Step 3:

2Li + Br₂ → 2LiBr

left hand side Right hand side

Li = 2 Li = 2

Br = 2 Br = 2

3 0

3 years ago

In the background information, it was stated that CaF2 has solubility, at room temperature, of 0.00160 g per 100 g of water. How

____ [38]

Answer:

2.05*10⁻⁵ moles of CF₂ can dissolve in 100 g of water.

12.82 moles of CaF₂ will dissolve in exactly 1.00 L of solution

Explanation:

First, by definition of solubility, in 100 g of water there are 0.0016 g of CaF₂. So, to know how many moles are 0.0016 g, you must know the molar mass of the compound. For that you know:

Ca: 40 g/mole
F: 19 g/mole

So the molar mass of CaF₂ is:

CaF₂= 40 g/mole + 2*19 g/mole= 78 g/mole

Now you can apply the following rule of three: if there are 78 grams of CaF₂ in 1 mole, in 0.0016 grams of the compound how many moles are there?

$moles=\frac{0.0016 grams*1 mole}{78 grams}$

moles=2.05*10⁻⁵

2.05*10⁻⁵ moles of CF₂ can dissolve in 100 g of water.

Now, to answer the following question, you can apply the following rule of three: if by definition of density in 1 mL there is 1 g of CaF₂, in 1000 mL (where 1L = 1000mL) how much mass of the compound is there?

$mass of CaF_{2}=\frac{1000 mL*1g}{1mL}$

mass of CaF₂= 1000 g

Now you can apply the following rule of three: if there are 78 grams of CaF₂ in 1 mole, in 1000 grams of the compound how many moles are there?

$moles=\frac{1000 grams*1 mole}{78 grams}$

moles=12.82

12.82 moles of CaF₂ will dissolve in exactly 1.00 L of solution

5 0

3 years ago