Given these reactions:

Which substance will require more energy to heat if all the samples have the same mass? A chart with two columns and nine rows.

Paraphin [41]

Here we have to identify the sample which need more energy to heat the sample 1 degree Celsius.

Among the given elements magnesium will require more energy than the others to heat.

As per the definition of specific heat of a compound, the amount of heat required to increase the temperature of the material 1 degree Celsius is the specific heat of the material.

The given data are-

substance specific heat

Lead 0.129

Tin 0.21

Silver 0.235

Iron 0.449

Calcium 0.647

Granite 0.803

Aluminium 0.897

Magnesium 1.023

From the given data lead, magnesium, iron and aluminium have the specific heat 0.129, 1.023, 0.449 and 0.897 respectively. Thus magnesium will require more energy than the others to heat.

6 0

3 years ago

When calcium carbonate is added to hydrochloric acid, calcium chloride, carbon dioxide, and water are produced. CaCO3 ( s ) + 2

BigorU [14]

Answer:

19.7 g of CaCl₂ are produced in the reaction

Explanation:

In this excersise we need to know the limiting reactant in order to determine the mass produced of a one of the products

The reaction is: CaCO₃ (s) + 2HCl (aq) → CaCl₂(aq) + H₂O (l) + CO₂(g)

First of all we must find the limiting reactant. For that purpose, we convert the mass of reactants to moles

25 g / 100.08 g/mol = 0.249 moles of carbonate

13 g / 36.45 g/mol = 0.357 moles of HCl

We work with the stoichiometry of the reaction:

1 mol of carbonate reacts with 2 moles of hydrochloric

Then, 0.249 moles of carbonate must react with (0.249 . 2) /1 = 0.498 moles of HCl (We do not have enough HCl, so this is the limtiing reactant)

We work with the stoichiometry reactant / product

2 moles of HCl can produce 1 mol of CaCl₂

Therefore 0.357 moles of HCl must produce (0.357 .1) / 2 = 0.178 moles of chloride.

We convert the moles to mass → 0.178 mol . 110.98 g /1mol = 19.7g

5 0

3 years ago

A 29.00 mL sample of an unknown H3PO4 solution is titrated with a 0.130 M NaOH solution. The equivalence point is reached when 2

beks73 [17]

I am first assuming that you want the molarity of the acid. Use the formula $M_{a} V_{a} = M_{b}V_{b}$ which is the titration formula. M is molarity (a is of acid and b is of base) and V is volume in mL (a is of acid and b is of base). Plugging in gives us $(29 mL)(M_{a}) = (0.130 M)(27.73 mL)$ . Solving gives us $M_{a} = 0.124 M$

6 0

3 years ago

What are possible components of ionic

Mekhanik [1.2K]

Answer: a metal and a nonmental and a mental and a polyatomic anion :)

Explanation: i prayed ~.~

4 0

3 years ago

Read 2 more answers

A piece of sodium metal reacts completely with water to produce sodium hydroxide and hydrogen gas. the hydrogen gas generated is

Evgesh-ka [11]

We get the pressure of the hydrogen gas from the difference between the measured pressure and the vapor pressure of water:
total pressure = Pressure of H2 + Vapor Pressure of H2O
1.00 atm = Pressure of H2 + 0.0313 atm
Pressure of H2 = 1.00 atm - 0.0313 atm = 0.9687 atm

From the ideal gas law,
PV = nRT
we can calculate for the number of moles of H2 as
n = PV/RT = (0.9687 atm)(0.246L) / (0.08206 L·atm/mol·K)(298.15 K)
= 0.00974 mol H2
where
V = 246 mL (1 L / 1000 mL) = 0.246 L
T = 25 degrees Celsius + 273.15 = 298.15 K

We use the mole ratio of Na and H2 from the reaction of sodium metal with water as shown in the equation
2Na(s) + 2H2O(l) → 2 NaOH(aq) + H2(g)
and the molar mass of sodium Na to get the mass of sodium used in the reaction:
mass of Na = 0.00974 mol H2 (2 mol Na /1 mol H2)(22.99 g Na/1 mol Na)
= 0.448 grams of sodium

4 0

3 years ago