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fenix001 [56]
1 year ago
15

a sample of mass 6.814grams is added to another sample weighing 0.08753 grams. the subsequent mixture is then divided into exact

ly 3 equal parts. one of those parts has the yield multiplied by 7.6335 times, what is the final mass?
Chemistry
1 answer:
Alexxx [7]1 year ago
6 0

Answer:

Final\ Mass = 17.560943085g

Explanation:

Given

Sample\ Mass = 6.814g

Additional\ Mass = 0.08753g

Yield = 7.6335

Required

Determine the final mass

First we need to determine the total mass after the sample mass is added to an additional sample;

Total\ Mass = Additional\ Mass + Sample\ Mass

Total\ Mass = 0.08753g + 6.814g

Total\ Mass = 6.90153g

Next, divide the total mass by 3

New\ Mass = \frac{Total\ Mass}{3}

New\ Mass = \frac{6.90153g}{3}

New\ Mass = 2.30051g

The final mass is calculated as follows;

Final\ Mass = New\ Mass * Yield

Final\ Mass = 2.30051g * 7.6335

Final\ Mass = 17.560943085g

<em>Hence, the final mass is 17.560943085g</em>

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4.82 g of an unknown metal is heated to 115.0∘C and then placed in 35 mL of water at 28.7∘C, which then heats up to 34.5∘C. What
nikitadnepr [17]

<u>Answer:</u> The specific heat of metal is 2.34 J/g°C

<u>Explanation:</u>

To calculate the mass of water, we use the equation:

\text{Density of substance}=\frac{\text{Mass of substance}}{\text{Volume of substance}}

Density of water = 1 g/mL

Volume of water = 35 mL

Putting values in above equation, we get:

1g/mL=\frac{\text{Mass of water}}{35mL}\\\\\text{Mass of water}=(1g/mL\times 35mL)=35g

When metal is dipped in water, the amount of heat released by metal will be equal to the amount of heat absorbed by water.

Heat_{\text{absorbed}}=Heat_{\text{released}}

The equation used to calculate heat released or absorbed follows:

Q=m\times c\times \Delta T=m\times c\times (T_{final}-T_{initial})

m_1\times c_1\times (T_{final}-T_1)=-[m_2\times c_2\times (T_{final}-T_2)]      ......(1)

where,

q = heat absorbed or released

m_1 = mass of metal = 4.82 g

m_2 = mass of water = 35 g

T_{final} = final temperature = 34.5°C

T_1 = initial temperature of metal = 115°C

T_2 = initial temperature of water = 28.7°C

c_1 = specific heat of metal = ?

c_2 = specific heat of water = 4.186 J/g°C

Putting values in equation 1, we get:

4.82\times c_1\times (34.5-110)=-[35\times 4.186\times (34.5-28.7)]

c_1=2.34J/g^oC

Hence, the specific heat of metal is 2.34 J/g°C

4 0
1 year ago
An old sample of concentrated sulfuric acid to be used in the laboratory is approximately 98.1 percent h2so4 by mass. calculate
Airida [17]
Basis: 100 mL solution

From the given density, we calculate for the mass of the solution.

                        density  = mass / volume
                        mass = density x volume

                       mass = (1.83 g/mL) x (100 mL) = 183 grams

Then, we calculate for the mass H2SO4 given the percentage.
                   
                      mass of H2SO4 = (183 grams) x (0.981) = 179.523 grams

Calculate for the number of moles of H2SO4,
                  moles H2SO4 = (179.523 grams) / (98.079 g/mol)
                        moles H2SO4 = 1.83 moles

Molarity:
                     M = moles H2SO4 / volume solution (in L)
                         = 1.83 moles / (0.1L ) = 18.3 M

Molality:
                     m = moles of H2SO4 / kg of solvent
                        = 1.83 moles / (183 g)(1-0.983)(1 kg/ 1000 g) = 588.24 m
8 0
2 years ago
A 63.5 g sample of an unidentified metal absorbs 355 ) of heat when its temperature changes
insens350 [35]

0.208 is the specific heat capacity of the metal.

Explanation:

Given:

mass (m)  = 63.5 grams 0R 0.0635 kg

Heat absorbed (q) = 355 Joules

Δ T (change in temperature) = 4.56 degrees or 273.15+4.56 = 268.59 K

cp (specific heat capacity) = ?

the formula used for heat absorbed  and to calculate specific heat capacity of a substance will be calculated by using the equation:

q = mc Δ T

c = \frac{q}{mΔ T}

c = \frac{355}{63.5X 268.59}

 = 0.208 J/gm K

specific heat capacity of 0.208 J/gm K

The specific heat capacity is defined as  the heat required to raise the temperature of a substance which is 1 gram. The temperature is in Kelvin and energy required is in joules.

 

5 0
2 years ago
Arranges the following molecules in order of increasing dipole moment: <br> H2O, H2S, H2Te, H2Se.
erastova [34]

Explanation:

Dipole moment is defined as the measurement of the separation of two opposite electrical charges.

H_{2}O is a bent shaped molecule with a dipole moment of 1.87.

H_{2}S is also a bent shaped molecule with a dipole moment of 1.10.

H_{2}Te is a also a bent shaped molecule and has a negligible dipole moment.

H_{2}Se has a dipole moment of 0.29.

Therefore, given molecules are arranged according to their increasing dipole moment as follows.

        H_{2}Te < H_{2}Se < H_{2}S < H_{2}O

7 0
2 years ago
Calculate the number of grams of xenon in 4.658 g of the compound xenon tetrafluoride.
andrezito [222]

Answer:

The mass of xenon in the compound is 2.950 grams

Explanation:

Step 1: Data given

Mass of XeF4 = 4.658 grams

Molar mass of XeF4 = 207.28 g/mol

Step 2: Calculate moles of XeF4

Moles XeF4 = mass XeF4 / molar mass XeF4

Moles XeF4 = 4.658 grams / 207.28 g/mol

Moles XeF4 = 0.02247 moles

Step 3: Calculate moles of xenon

XeF4 → Xe + 4F-

For 1 mol xenon tetrafluoride, we have 1 mol of xenon

For 0.02247 moles XeF4 we have 0.02247 moles Xe

Step 4: Calculate mass of xenon

Mass xenon = moles xenon * molar mass xenon

Mass xenon = 0.02247 moles * 131.29 g/mol

Mass xenon = 2.950 grams

The mass of xenon in the compound is 2.950 grams

5 0
2 years ago
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