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3 years ago

Write balanced complete ionic equation for K2SO4(aq)+CaI2(aq)→CaSO4(s)+KI(aq)

2 answers:

7 0

CaSO4(s) might be an improperly capitalized: CAsO4(S), CaSO4(S) Balanced equation: K2SO4(aq) + CaI2(aq) = CaSO4(s) + 2 KI(aq) Reaction type: double replacement.

german3 years ago

3 0

For ionic equation, the ions that are not involved in the reaction will be deleted. In this equation, the K+ and I- ion are not involved. So the answer should be SO42+(aq) + Ca2+(aq) -> CaSO4(s).

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Calculate the solubility of hydrogen in water at an atmospheric pressure of 0.380 atm (a typical value at high altitude).

Pani-rosa [81]

The question is incomplete, here is the complete question:

Calculate the solubility of hydrogen in water at an atmospheric pressure of 0.380 atm (a typical value at high altitude).

Atmospheric Gas Mole Fraction kH mol/(L*atm)

$N_2$ $7.81\times 10^{-1}$ $6.70\times 10^{-4}$

$O_2$ $2.10\times 10^{-1}$ $1.30\times 10^{-3}$

Ar $9.34\times 10^{-3}$ $1.40\times 10^{-3}$

$CO_2$ $3.33\times 10^{-4}$ $3.50\times 10^{-2}$

$CH_4$ $2.00\times 10^{-6}$ $1.40\times 10^{-3}$

$H_2$ $5.00\times 10^{-7}$ $7.80\times 10^{-4}$

<u>Answer:</u> The solubility of hydrogen gas in water at given atmospheric pressure is $1.48\times 10^{-10}M$

<u>Explanation:</u>

To calculate the partial pressure of hydrogen gas, we use the equation given by Raoult's law, which is:

$p_{\text{hydrogen gas}}=p_T\times \chi_{\text{hydrogen gas}}$

where,

$p_A$ = partial pressure of hydrogen gas = ?

$p_T$ = total pressure = 0.380 atm

$\chi_A$ = mole fraction of hydrogen gas = $5.00\times 10^{-7}$

Putting values in above equation, we get:

$p_{\text{hydrogen gas}}=0.380\times 5.00\times 10^{-7}\\\\p_{\text{hydrogen gas}}=1.9\times 10^{-7}atm$

To calculate the molar solubility, we use the equation given by Henry's law, which is:

$C_{H_2}=K_H\times p_{H_2}$

where,

$K_H$ = Henry's constant = $7.80\times 10^{-4}mol/L.atm$

$p_{H_2}$ = partial pressure of hydrogen gas = $1.9\times 10^{-7}atm$

Putting values in above equation, we get:

$C_{H_2}=7.80\times 10^{-4}mol/L.atm\times 1.9\times 10^{-7}atm\\\\C_{CO_2}=1.48\times 10^{-10}M$

Hence, the solubility of hydrogen gas in water at given atmospheric pressure is $1.48\times 10^{-10}M$

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2 years ago

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Kamila [148]

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2 years ago

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How many grams of chromium are in 2.0 x 1024 atoms

Vaselesa [24]

Answer: 173 g ( 0.17 kg in right accuracy)

Explanation: Amount in moles is n = N/Na = 2.0·10^24 / 6.022·10^23 (1/mol).

n = 3.32116 mol. M(Cr) = 52.00 g/mol and mass m = nM = 172.7 g

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A force of attraction that holds atom together
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