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umka2103 [35]
3 years ago
15

How can a student collect and measure the volume of a gas produced ?

Chemistry
1 answer:
Anastasy [175]3 years ago
8 0

The volume of oxygen produced can be measured using the gas syringe method. The gas collects in the syringe, pushing out against the plunger. The volume of gas that has been produced can be read from the markings on the syringe.

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134 miles= ? inches. Chemistry
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3 0
3 years ago
Read 2 more answers
ASAP , 8.81 g Carbon
xz_007 [3.2K]

The empirical formula : C₂Cl₇

The molecular formula : C₁₀Cl₃₅

<h3>Further explanation</h3>

Given

8.81 g Carbon

91.2 g Chlorine

Molar Mass: 1362.5 g/mol

Required

The empirical formula and molecular formula

Solution

Mol ratio :

C = 8.81 g : 12.011 g/mol =0.733

Cl = 91.2 g : 35,453 g/mol = 2..572

Divide by 0.733

C : Cl = 1 : 3.5 = 2 : 7

The empirical formula : C₂Cl₇

(The empirical formula)n = the molecular formula

(C₂Cl₇)n = 1362.5

(2x12.011+7x35.453)n=1362.5

(272.193)n=1362.5

n = 5

6 0
3 years ago
The gases carbon dioxide, oxygen, and argon are mixed in a container. All gases have the same partial pressure, and the total pr
polet [3.4K]
The partial pressure of argon can be calculated simply by dividing the total pressure by 3. This gives an answer equivalent to 10893.33 Pa. The clue behind this is the statement "a<span>ll gases have the same partial pressure". This follows Dalton's Law of Partial Pressures which states that the total pressure is equal to the sum of the individual partial pressures.</span>
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3 years ago
What is the name of the compound in cabbage juice that causes the color to change in an acid or base?
baherus [9]
Red cabbage contains a water-soluble pigment called anthocyanin<span> that changes color when it is mixed with an acid or a base. The pigment turns red in acidic environments with a pH less than 7 and the pigment turns bluish-green in alkaline (basic) environments with a pH greater than 7.</span>
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3 years ago
Suppose 215 g of NO3- flows into a swamp each day. What volume of CO2 would be produced each day at 17.0°C and 1.00 atm?
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Answer:

The answer is "41.23 \ L\  N_2"

Explanation:

2 NO_3^{-} + 10 e^{-} + 12 H^{+} \longrightarrow N_2 + 6 H_2O\\\\= \frac{( 215 \ g \ NO_3^{-})}{(62.0049  \frac{\ g NO_3^{-}}{mol})} \times  \frac{(1 \ mol \ N_2}{ 2 \ mol \ NO_3^{-})}\\\\

=3.46746789 \times 0.5\\\\= 1.733 \ mol \ N_2 \\\\\to V = \frac{nRT}{P} \\\\= (1.733 \ mol) \times (0.08205746 \frac{L\ atm}{Kmol}) \times \frac{ (17 + 273) K}{(1.00 atm)}\\\\= 41.23

8 0
3 years ago
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