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7 days ago

If 3.491 grams of the precipitate was formed, how many moles of strontium bromide were reacted

1 answer:

4 0

The chemical reaction can be expressed with this balanced equation:
<span>SrBr2(aq) + 2AgNO3(aq) → Sr(NO3)2(aq) + 2AgBr(s)
</span>
Using the periodic table:
Silver has a mass of 108 grams
Bromine weighs 80 grams

Thus, the molar mass of silver bromide amounts to 188 grams (108 + 80).

To find the number of moles, we use the formula: number of moles = mass / molar mass
The moles of precipitate formed can be calculated as 3.491/188 = 0.018 moles.

According to the balanced equation:
1 mole of strontium bromide gives rise to 2 moles of silver bromide. Therefore, we can find the moles of strontium bromide required to create 0.018 moles of silver bromide by cross-multiplying as follows:
amount of<span>strontium bromide = (0.018x1) / 2 = 9.28 x 10^-3 moles</span>

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What is the molar mass of citric acid (C6H8O7) and baking soda (NaHCO3)?

Alekssandra [992]

Answer:

1. 192.0 g/mol.

2. 84.0 g/mol.

Explanation:

The molar mass refers to the weight of all atoms combined in a molecule measured in grams per mole.

To find a molecule's molar mass, we begin by looking up the atomic weights of the relevant elements from the periodic table. Next, we tally the atoms present and multiply that by their respective atomic weights.

1. Molar mass of citric acid (C₆H₈O₇):

Molar mass of C₆H₈O₇ = 6(atomic mass of C) + 8(atomic mass of H) + 7(atomic mass of O) = 6(12.0 g/mol) + 8(1.0 g/mol) + 7(16.0 g/mol) = 192.0 g/mol.

2. Molar mass of baking soda (NaHCO₃):

Molar mass of NaHCO₃ = (atomic mass of Na) + (atomic mass of H) + (atomic mass of C) + 3(atomic mass of O) = (23.0 g/mol) + (1.0 g/mol) + (12.0 g/mol) + 3(16.0 g/mol) = 84.0 g/mol.

4 0

2 days ago

An infant acetaminophen suspension contains 80 mg/0.80 mL suspension. The recommended dose is 15 mg/kg body weight.

KiRa [976]

Response:

0.8853 mL

Clarification:

Initially, we convert 13 lb to kg, remembering that 1 lb = 0.454 kg:

13 lb * $\frac{0.454kg}{1lb}$ = 5.902 kg

Next, we determine the required mg of acetaminophen to administer, applying the recommended dosage and infant's weight:

15 mg/kg * 5.902 kg = 88.53 mg

Finally, we compute the necessary mL of suspension, utilizing its concentration:

88.53 mg ÷ (80 mg/0.80 mL) = 0.8853 mL

8 0

7 days ago

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

lions [1003]

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

3 0

1 day ago

The ionic radius of a sodium ion is 2.27 angstroms (A) . What is this length in um

lions [1003]

$\boxed{\sf 1Å=10^{-10}m}$

$\\ \rm\longmapsto 2.27Å$

$\\ \rm\longmapsto 2.27\times 10^{-10}m$

$\\ \rm\longmapsto 0.227\times 10^{-9}m$

$\\ \rm\longmapsto 0.0227\times 10^{-8}m$

$\\ \rm\longmapsto 0.00227\times 10^{-7}m$

$\\ \rm\longmapsto 0.00023\times 10^{-6}m$

$\\ \rm\longmapsto 0.00023\mu m$

6 0

12 days ago

The concentration of Si in an Fe-Si alloy is 0.25 wt%. What is the concentration in kilograms of Si per cubic meter of alloy?

KiRa [976]

Answer: The mass of Si in kilograms is, $19.55kg/m^3$

Explanation:

Given that the Si concentration in an Fe-Si alloy is 0.25 weight percent, this translates to:

Mass of Si = 0.25 g = 0.00025 kg

Mass of Fe = 100 - 0.25 = 99.75 g = 0.09975 kg

Density of Si = $2.32g/cm^3=2.32\times 10^6g/m^3$

Density of Fe = $7.87g/cm^3=7.87\times 10^6g/m^3$

Next, we need to find the quantity of Si in kilograms per cubic meter of alloy.

Si concentration in kilograms = $\frac{\text{Weight of Si in 100 g of alloy}}{\text{Volume of 100 g of alloy}}$

Si concentration in kilograms = $\frac{\text{Weight of Si in 100 g of alloy}}{\frac{\text{Wight of Fe}}{\text{Density of Fe}}+\frac{\text{Wight of Si}}{\text{Density of Si}}}$

By substituting all the provided values into this formula, we arrive at:

Si concentration in kilograms = $\frac{0.00025kg}{\frac{99.75g}{7.87\times 10^6g/m^3}+\frac{0.25g}{2.23\times 10^6g/m^3}}$

Si concentration in kilograms = $19.55kg/m^3$

Hence, the mass of Si in kilograms is, $19.55kg/m^3$

5 0

8 days ago