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Ksju [112]
2 years ago
10

Which statement defines specific heat capacity for a given sample

Chemistry
1 answer:
avanturin [10]2 years ago
8 0

The statement that defines the specific heat capacity for a given sample is the quantity of heat that is required to raise 1 g of the sample by 1°C (Kelvin) at a constant pressure.

<h3>What is specific heat capacity?</h3>

Specific heat capacity is the of heat to increase the temperature per unit mass.

The formula to calculate the specific heat is Q = mct.

The options are attached here:

  1. The temperature of a given sample is 1 %.
  2. The temperature that a given sample can withstand.
  3. The quantity of heat that is required to raise the sample's temperature by 1 °C1 °C (Kelvin).
  4. The quantity of heat that is required to raise 1 g of the sample by 1°C (Kelvin) at a constant pressure.

Thus, the correct option is 4. The quantity of heat that is required to raise 1 g of the sample by 1°C (Kelvin) at a constant pressure.

Learn more about specific heat capacity

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21-B. Mn was used as an internal standard for measuring Fe by atomic absorption. A standard mixture containing 2.00 mg Mn/mL and
Korvikt [17]

Answer:

0.0693M Fe

Explanation:

It is possible to quantify Fe in a sample using Mn as internal standard using response factor formula:

F = A(analyte)×C(std) / A(std)×C(analyte) <em>(1)</em>

Where A is area of analyte and std, and C is concentration.

Replacing with first values:

F = 1.05×2.00mg/mL / 1.00×2.50mg/mL

<em>F = 0.84</em>

In the unknown solution, concentration of Mn is:

13.5mg/mL × (1.00mL/6.00mL) = <em>2.25 mg Mn/mL</em>

Replacing in (1) with absorbances values and F value:

0.84 = 0.185×2.25mg/mL / 0.128×C(analyte)

C(analyte) = <em>3.87 mg Fe / mL</em>

As molarity is moles of solute (Fe) per liter of solution:

\frac{3.87 mg Fe}{mL} \frac{1g}{1000mg} \frac{1mol}{55.845g} \frac{1000mL}{1L} = <em>0.0693M Fe</em>

7 0
3 years ago
Read 2 more answers
Samira has two pens. She wants to know which pen was used to write a note. She labels her pens A and B. She puts a sample of ink
Ann [662]

Answer:

b

Explanation:

8 0
3 years ago
Manganese commonly occurs in nature as a mineral. The extraction of manganese from the carbonite mineral rhodochrosite, involves
hjlf

This is an incomplete question, here is a complete question.

Manganese commonly occurs in nature as a mineral. The extraction of manganese from the carbonite mineral rhodochrosite, involves a two-step process. In the first step, manganese (II) carbonate and oxygen react to form manganese (IV) oxide and carbon dioxide:

2MnCO_3(s)+O_2(g)\rightarrow 2MnO_2(s)+2CO_2(g)

In the second step, manganese (IV) oxide and aluminum react to form manganese and aluminum oxide:

3MnO_2(s)+4Al(s)\rightarrow 3Mn(s)+2Al_2O_3(s)

Write the net chemical equation for the production of manganese from manganese (II) carbonate, oxygen and aluminum. Be sure your equation is balanced.

Answer : The net chemical equation for the production of manganese is:

6MnCO_3(s)+3O_2(g)+8Al(s)\rightarrow 6CO_2(g)+6Mn(s)+4Al_2O_3(s)

Explanation :

The given two chemical reactions are:

(1) 2MnCO_3(s)+O_2(g)\rightarrow 2MnO_2(s)+2CO_2(g)

(2) 3MnO_2(s)+4Al(s)\rightarrow 3Mn(s)+2Al_2O_3(s)

First we are multiplying reaction 1 by 3, and reaction 2 by 2, we get:

(1)

(2) 6MnO_2(s)+8Al(s)\rightarrow 6Mn(s)+4Al_2O_3(s)

Now we are adding both the reactions, we get the overall chemical reaction.

6MnCO_3(s)+3O_2(g)+6MnO_2(s)+8Al(s)\rightarrow 6MnO_2(s)+6CO_2(g)+6Mn(s)+4Al_2O_3(s)

The  MnO_2 is common on both side, by cancelling it, we get:

The net chemical equation for the production of manganese is:

6MnCO_3(s)+3O_2(g)+8Al(s)\rightarrow 6CO_2(g)+6Mn(s)+4Al_2O_3(s)

5 0
3 years ago
Determine the acid dissociation constant for a 0.0250 M weak acid solution that has a pH of 2.37 . The equilibrium equation of i
Oksanka [162]

Answer:

For part (a): pHsol=2.22

Explanation:

I will show you how to solve part (a), so that you can use this example to solve part (b) on your own.

So, you're dealing with formic acid, HCOOH, a weak acid that does not dissociate completely in aqueous solution. This means that an equilibrium will be established between the unionized and ionized forms of the acid.

You can use an ICE table and the initial concentration ofthe acid to determine the concentrations of the conjugate base and of the hydronium ions tha are produced when the acid ionizes

HCOOH(aq]+H2O(l]⇌ HCOO−(aq] + H3O+(aq]

I 0.20 0 0

C (−x) (+x) (+x)

E (0.20−x) x x

You need to use the acid's pKa to determine its acid dissociation constant, Ka, which is equal to

3 0
2 years ago
Cuanto pesan 2 moles de HCI
maks197457 [2]

Answer:

FORMULA: HCl PESO MOLECULAR: 36.46 g/mol COMPOSICION: Cl: 97.23 % y H: 2.76 %. GENERALIDADES: El ácido clorhídrico es una disolución acuosa de cloruro de hidrógeno.

5 0
3 years ago
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