Answer:
Explanation:1 mole is equal to 1 moles CaCO3, or 100.0869 grams.
Answer:
Everything that has mass and takes up space is matter. Every day, you encounter phenomena that either don't have mass or don't take up space. They are non-matter. Basically, any type of energy or any abstract concept is an example of something that is not matter.
An apple.
A person.
A table.
Air.
Water.
A computer.
Paper.
Iron.
hope this helped you
Answer:The mineral that reacts to hydrochloric acid (HCl) only when powdered is calcite. Calcite is a carbonate mineral composed of calcium carbonate (CaCO3). When calcite is in its powdered form, it readily reacts with hydrochloric acid to produce carbon dioxide (CO2), water (H2O), and calcium chloride (CaCl2). This reaction can be described by the chemical equation:
CaCO3 (s) + 2HCl (aq) → CO2 (g) + H2O (l) + CaCl2 (aq)
The reaction occurs because the surface area of the powdered calcite is increased, allowing for a greater contact area between the mineral and the hydrochloric acid. This increased contact area facilitates a faster and more vigorous reaction compared to when the calcite is in its solid, non-powdered form.
It's important to note that not all minerals react with hydrochloric acid. Only minerals that contain carbonate ions (CO3^2-) will react with hydrochloric acid to produce carbon dioxide gas. Other common minerals that exhibit this reaction include limestone and marble, which also contain calcium carbonate.
By understanding this reaction and its characteristics, you can identify calcite and other carbonate-containing minerals by their reaction to hydrochloric acid when in powdered form.
Calcite is a mineral that reacts to hydrochloric acid (HCl) only when powdered. This reaction produces carbon dioxide gas.
The mineral that reacts to hydrochloric acid (HCl) only when powdered is calcite.
When solid calcite is exposed to hydrochloric acid, it does not undergo any noticeable reaction. However, when powdered calcite is mixed with HCl, it readily fizzes and releases carbon dioxide gas.
This reaction occurs because the acid dissolves the calcite, converting it into dissolved calcium ions and carbon dioxide gas.
Learn more about Calcite mineral reaction with hydrochloric acid here:
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Answer:
C: water crops often to wet soil.
Explanation:
Working in the plan industry, it becomes obvious that when watering the plants often, it will pack down the topsoil into the plant. Topsoil is lose at first as stated above, but when enough water gets on it, it becomes almost like mud. This is the kind of topsoil you want. No wind or water will mess it up because it already it watered! It will also help the grow. In addition, plowing is not correct because you only need to plow twice in the plant process. Before you plant the seeds, and to harvest the crops. If you plow to soon and often, you won’t have any plants.
B. depolymerization
C. digestion
D. cellular respiration
Answer: Cellular Respiration
Explanation:
The cellular respiration can be defined as the biological process by which the organism get energy to do work or to perform the various metabolic processes of the body.
The glucose produced by the plants is utilized in the process of cellular respiration where the glucose is broken down in pressence of oxygen to provide energy for various body functions.
The correct answer would be the letter D, Cellular respiration.
Cellular respiration allows the production of ATP through the breakdown of glucose assisted by oxygen. We talk about aerobic metabolism. This metabolism is to oppose the fermentation which is done without oxygen (anaerobic) and that we detail in another file. Cellular respiration is divided into two phases, one cytoplasmic and the other mitochondrial.
Answer:
Second order
Δ[ClO⁻]/Δt = - 4.183 x 10⁻⁴ M/min
Explanation:
Given the data:
Experiment # [ClO–] (M) Initial Rate of Formation of ClO3– (M/min)
1 10.452 1.048 x 10⁻⁴
2 20.903 4.183 x 10⁻⁴
we need to determine the order of the reaction with respect to ClO⁻.
We know the rate law for this reaction will have the form:
Rate = k [ClO⁻]^n
where n is the order of the reaction. Thus, what we need to do is to study the dependence of the initial rate on n for the experiment.
If the reaction were zeroth order the rate would not change, so we can eliminate n= 0
If the reaction were first order, doubling the concentration of [ClO–] , as it was done exactly in experiment # 2, the initial rate should have doubled, which is not the case.
If the reaction were second order n: 2, doubling the concentration of [ClO–] , should quadruple the initial rate of formation of ClO3–, which is what it is observed experimentally. Therefore the reaction is second order respect to ClO–.
The initial rate of consumption of ClO⁻ is the same as the rate of formation of ClO₃⁻ since:
Δ = - Δ[ClO⁻]/Δt = + Δ[ClO₃⁻]/Δt = + 1/2 [Cl⁻] /Δt
where t is the time.
from the coefficients of the balanced chemical equation.
- Δ[ClO⁻]/Δt = + Δ[ClO₃⁻]/Δt = + 1/2 [Cl⁻ ] = rate
Δ[ClO⁻]/Δt = - 4.183 x 10⁻⁴ M/min
B. 1/1 H
C. 0/1 H
D. 2/1 H