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1 month ago

3. For the reaction: 2X + 3Y 3Z, the combination of 2.00 moles of X with 2.00

Chemistry

1 answer:

lions [2.9K]1 month ago

3 0

Answer:

Explanation:

Considering the reaction: 2X + 3Y = 3Z, combining 2.00 moles of X with 2.00 moles of Y results in the production of 1.75 moles of Z.

2 mol 2 mol 1.75 mol

2X + 3Y = 3Z

2 mol is required with 3 mol to yield 3 mol.

3 mol Z / 3 mol Y = 1 to 1

should yield 2 mol Z

1.75 / 2 = 87.5 % production yield

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How many carbon atoms are contained in 84.3 g of ethyne (c2h2)?

alisha [2963]

<span>To find the number of carbon atoms, begin by eliminating grams from the given 84.3 g of C2H2 by dividing it by ethyne's molar mass, which is 26.038 g/mol. This molar mass is computed by summing the atomic masses of 2 carbons (12.011 g/mol each) and 2 hydrogens (1.008 g/mol each). This calculation yields the amount in moles of ethyne. Then, multiply by Avogadro's constant (6.022x10^23 atoms/mol) to convert moles of ethyne to atoms of ethyne. Since each C2H2 molecule contains 2 carbon atoms, multiply by 2 carbon atoms per ethyne molecule to get the total carbon atoms, resulting in 3.90x10^24 atoms of carbon. This figure is rounded to three significant digits, consistent with the smallest number of significant figures (three in 84.3). The steps are: 84.3 g C2H2 × (1 mol C2H2 / 26.038 g C2H2) × (6.022×10^23 atoms C2H2 / 1 mol C2H2) × (2 atoms C / 1 atom C2H2) = 3.90×10^24 carbon atoms.</span>

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1 month ago

11mg of cyanide per kilogram of body weight is lethal for 50% of domestic chickens. If a chicken weighs 3kg, how many grams of c

lions [2927]

Answer:

$0.033g$

Explanation:

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In this scenario, since 11 mg of cyanide per kilogram of body weight is lethal for 50% of domestic chickens, we can determine the lethal amount for a chicken weighing 3 kg using a proportion:

$11mg\longrightarrow 1kg\\\\?\ \ \ \ \ \ \longrightarrow 3kg$

Thus, we find:

$?=\frac{3kg*11mg}{1kg}\\ \\?=33mg$

Which equates to grams as follows:

$=33mg*\frac{1g}{1000mg} \\\\=0.033g$

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16 days ago

1.562 g sample of the alcohol CH3CHOHCH2CH3 is burned in an excess of oxygen. What masses of H2O and CO2 should be obtained

eduard [2782]

Answer:

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Explanation:

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In this scenario, as the molecular formula for the specified alcohol is C₄H₁₀O (with a molar mass of 74.14 g/mol), its combustion reaction can be represented as follows:

$C_4H_1_0O+6O_2\rightarrow 4CO_2+5H_2O$

This implies a mole ratio of 1:4 with carbon dioxide (molar mass = 44.01 g/mol) and a mole ratio of 1:5 with water (molar mass = 18.02 g/mol), allowing us to determine the resultant masses as follows:

$m_{CO_2}=1.562gC_4H_1_0O*\frac{1mol}{74.14gC_4H_1_0O} *\frac{4molCO_2}{1molC_4H_1_0O} *\frac{44.01gCO_2}{1molCO_2}=3.709gCO_2 \\\\m_{H_2O}=1.562gC_4H_1_0O*\frac{1mol}{74.14gC_4H_1_0O} *\frac{5molH_2O}{1molC_4H_1_0O} *\frac{18.02gH_2O}{1molH_2O}=1.898gH_2O$

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1 month ago

How much heat is required, in calories, to raise the temperature of 57.8g of silver from 17.0oC to 43.5oC, if the specific heat

lorasvet [2795]

Response:

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Clarification:

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21 day ago

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alisha [2963]

Answer:

The equation formulated by Michaelis-Menten is expressed as

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Explanation:

Refer to the attached image for an in-depth clarification

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1 month ago